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QUESTION

Feb 03, 2017

How many moles of sodium hypobromite (NaBrO) must be added to a 2.00 L solution of 0.025 M hypobromous acid (HBrO) to form a buffer solution of pH 9.0 (Ka HBrO is 2.5x10-9)? Assume the volume of solution does not change on addition of NaBrO?

##"17 g"##

A must contain either a Weak acid and its conjugte base, or a weak base and its conjugate acid, in comparable amounts.

The idea here is that you need to determine how much sodium hypobromite, ##"NaBrO"##, is needed in order to supply enough hypobromite anions, the conjugate base of hypobromous acid, ##"HBrO"##, in order to form a buffer of equal to ##9##.

Your tool of choice here will be the Henderson - Hasselbalch equation for a weak acid - conjugate base buffer